To determine which atom has all electrons paired in the ground state, we need to examine the electron configuration of each atom.

Let's start with atom A, Ba (Barium). The electron configuration of Barium is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2. From this configuration, we can see that there are unpaired electrons in the 6s orbital.

Moving on to atom B, Br (Bromine). The electron configuration of Bromine is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^5. In this case, there is one unpaired electron in the 4p orbital.

Next, let's consider atom C, S (Sulfur). The electron configuration of Sulfur is 1s^2 2s^2 2p^6 3s^2 3p^4. Here, there are two unpaired electrons in the 3p orbital.

Now, let's move on to atom D, Si (Silicon). The electron configuration of Silicon is 1s^2 2s^2 2p^6 3s^2 3p^2. In this case, there are two unpaired electrons in the 3p orbital.

Based on our analysis, it can be concluded that none of the given atoms have all electrons paired in the ground state.

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To determine which atom has all electrons paired in the ground state, we need to examine the electron configuration of each atom.

Let's start with atom A, Ba (Barium). The electron configuration of Barium is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2. From this configuration, we can see that there are unpaired electrons in the 6s orbital.

Moving on to atom B, Br (Bromine). The electron configuration of Bromine is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^5. In this case, there is one unpaired electron in the 4p orbital.

Next, let's consider atom C, S (Sulfur). The electron configuration of Sulfur is 1s^2 2s^2 2p^6 3s^2 3p^4. Here, there are two unpaired electrons in the 3p orbital.

Now, let's move on to atom D, Si (Silicon). The electron configuration of Silicon is 1s^2 2s^2 2p^6 3s^2 3p^2. In this case, there are two unpaired electrons in the 3p orbital.

Based on our analysis, it can be concluded that none of the given atoms have all electrons paired in the ground state.

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To determine which atom has all electrons paired in the ground state, we need to examine the electron configuration of each atom.

Let's start with atom A, Ba (Barium). The electron configuration of Barium is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2. From this configuration, we can see that there are unpaired electrons in the 6s orbital.

Moving on to atom B, Br (Bromine). The electron configuration of Bromine is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^5. In this case, there is one unpaired electron in the 4p orbital.

Next, let's consider atom C, S (Sulfur). The electron configuration of Sulfur is 1s^2 2s^2 2p^6 3s^2 3p^4. Here, there are two unpaired electrons in the 3p orbital.

Now, let's move on to atom D, Si (Silicon). The electron configuration of Silicon is 1s^2 2s^2 2p^6 3s^2 3p^2. In this case, there are two unpaired electrons in the 3p orbital.

Based on our analysis, it can be concluded that none of the given atoms have all electrons paired in the ground state.

This question refers to isolated gaseous atoms in the ground state.In which atom are all electrons paired?A Ba B Br C S D Si

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